Podcast
Questions and Answers
What effect does increasing pressure have on a system at equilibrium?
What effect does increasing pressure have on a system at equilibrium?
A catalyst changes the position of the equilibrium in a reversible reaction.
A catalyst changes the position of the equilibrium in a reversible reaction.
False (B)
What is the key characteristic of a catalyst that remains unchanged during a chemical reaction?
What is the key characteristic of a catalyst that remains unchanged during a chemical reaction?
It does not undergo any permanent changes.
In heterogeneous catalysis, reaction molecules are _________ onto the surface of the catalyst.
In heterogeneous catalysis, reaction molecules are _________ onto the surface of the catalyst.
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Match the following catalysts with their respective applications:
Match the following catalysts with their respective applications:
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According to the Maxwell-Boltzmann distribution, how does a catalyst affect the activation energy?
According to the Maxwell-Boltzmann distribution, how does a catalyst affect the activation energy?
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At a dynamic equilibrium, the concentration of reactants and products are constantly changing.
At a dynamic equilibrium, the concentration of reactants and products are constantly changing.
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State Le Chatelier's principle in a sentence
State Le Chatelier's principle in a sentence
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When testing temperature effects on a reaction, cobalt chloride is dissolved in water, then a few drops of ________ are added to the boiling tube before investigation in a cold bath.
When testing temperature effects on a reaction, cobalt chloride is dissolved in water, then a few drops of ________ are added to the boiling tube before investigation in a cold bath.
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When adding ammonium hydroxide (NH₄OH) to a solution of yellow potassium chromate (K₂CrO₄) with sulfuric acid, what color change will occur?
When adding ammonium hydroxide (NH₄OH) to a solution of yellow potassium chromate (K₂CrO₄) with sulfuric acid, what color change will occur?
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Flashcards
Catalyst
Catalyst
A substance that increases the rate of a reaction without permanent change.
Homogeneous Catalyst
Homogeneous Catalyst
A catalyst that is in the same physical state as the reactants.
Heterogeneous Catalyst
Heterogeneous Catalyst
A catalyst that is in a different physical state than the reactants.
Activation Energy
Activation Energy
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Maxwell-Boltzmann Distribution
Maxwell-Boltzmann Distribution
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Dynamic Equilibrium
Dynamic Equilibrium
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Le Chatelier's Principle
Le Chatelier's Principle
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Pressure and Equilibrium
Pressure and Equilibrium
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Catalyst and Reaction Pathway
Catalyst and Reaction Pathway
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Effects of Temperature on Reaction Rate
Effects of Temperature on Reaction Rate
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Study Notes
Experimental Setup
- Boiling water bath set up for heating.
- Boiling tube transferred to it.
- Boiling tube moved back to cold water.
- Starting color: blue.
Catalysis and Equilibrium
- Increasing pressure shifts equilibrium to the side with fewer moles of gas to reduce pressure.
- Catalysts do not change equilibrium position, but instead increase reaction rate.
Catalysts
- Catalyst increases reaction rate without being consumed.
- May react with reactants to form intermediates.
- Provides an alternative pathway with lower activation energy.
Types of Catalysts
- Homogeneous catalyst: Same physical state as reactants (e.g., Cl radicals in ozone depletion).
- Heterogeneous catalyst: Different physical state (e.g., reactions on a surface).
- Reactants adsorb (weakly bind) to the catalyst surface.
- Reaction occurs on the surface.
- Products desorb (leave the surface).
Examples of Heterogeneous Catalysis
- Iron in the Haber process.
- Pt or Rh in reforming.
- Ni in alkene hydrogenation.
- V₂O₅ in sulfuric acid production.
Maxwell-Boltzmann Distribution
- Catalyst effect: Lower activation energy, allowing more molecules to react at a given temperature. Total molecules unchanged. Distribution shape remains similar.
- Without Catalyst:
- Curve starts from zero energy.
- Area under the curve = total number of molecules.
- No maximum molecule energy (curve doesn't hit the x-axis).
- Higher temperatures:
- More molecules exceed activation energy.
- Increased collision rate leads to faster reactions.
- Higher molecular kinetic energy meaning more collisions.
Dynamic Equilibrium & Le Chatelier's Principle
- Dynamic equilibrium: Forward and reverse reaction rates are equal. Reactant and product concentrations remain constant.
- Le Chatelier's principle: Equilibrium shifts to counteract changes.
- More product formation shifts equilibrium to the right.
- More reactant formation shifts equilibrium to the left.
Experimental Procedures - Investigating Concentration Changes
- Starting with yellow K₂CrO₄ solution + dilute H₂SO₄.
- Result: Orange solution.
- Adding NH₄OH turns it back to yellow.
Experimental Procedures - Investigating Temperature Effects
- Cobalt chloride dissolved in water.
- A few drops of HCl added.
- Observing color change in a boiling tube placed in an ice bath.
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Description
Explore the principles of catalysis and chemical equilibrium in this quiz. Understand the differences between homogeneous and heterogeneous catalysts, their roles in reactions, and the effect of pressure on equilibrium. Test your knowledge on key concepts and examples in catalytic processes.
